June 19, 2021, 12:04:09 AM
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Topic: How to standadize NaHCO3 using HCl  (Read 170 times)

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Offline aladin89

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How to standadize NaHCO3 using HCl
« on: June 01, 2021, 11:23:45 PM »
Hello everyone,
Im new to this group. I want to know titration method of standardization NaHCO3 using HCl.


Offline Borek

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Re: How to standadize NaHCO3 using HCl
« Reply #1 on: June 02, 2021, 03:13:49 AM »
Please read the forum rules. You have to show your attempts at answering the question/solving the problem to receive help, it is a forum policy.

This sounds like a classic acid/base titration. Check the endpoint pH to select the indicator
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info, pH-meter.info

Offline Elric82

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Re: How to standadize NaHCO3 using HCl
« Reply #2 on: June 02, 2021, 05:09:31 AM »
Hello everyone,
Im new to this group. I want to know titration method of standardization NaHCO3 using HCl.

Im assuming you have read the rules by now and know that an answer wont/cant be given.  But this can still be worked through.

So what do you know of titrations and molarity? Would you simply react a liquid with a solid, or would you make an aqueous solution?

Offline Asim

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Re: How to standadize NaHCO3 using HCl
« Reply #3 on: Yesterday at 04:19:05 PM »
A Two-Stage Reaction
When you add a hydrochloric acid (HCl) solution to a solution of sodium carbonate (Na2CO3), the hydrogen ion in HCl switches places with one of the sodium ions in Na2CO3 to produce sodium hydrogencarbonate, also known as sodium bicarbonate (baking soda), and sodium chloride (salt).

Na2CO3(aq) + HCl(aq) → NaHCO3(aq) + NaCl(aq)

Sodium hydrogencarbonate is basic, and it reacts with the HCl still in solution to produce sodium chloride, carbon dioxide and water.

NaHCO3(aq) + HCl(aq) → NaCl(aq) + CO2(g) + H2O(l)

Phenolphthalein is a good indicator for the first reaction because it responds to the pH change caused by the formation of sodium hydrogencarbonate. It is pink in basic solutions and turns colorless as soon as the solution becomes acidic. Methyl orange, on the other hand, responds to pH changes associated with the formation of NaCl, changing from yellow to red as the solution becomes more acidic. At neutrality, it is a distinct orange color


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